US2107857A - Process for oxidizing phosphorus - Google Patents

Description

Patented Feb. 8, 1938 PATENT OFFICE 2,107,857 PROCESS FOR OXIDIZING PHOSPHO-RUS Paul H. Emmett, Washington, D. 0., assignor to Henry A. Wallace, Secretary ofAgriculture of the United States of America No Drawing. Application June 7, 1937,

- Serial No. 146,851

4 Claims.

(Granted under the act March 3, 1883, as amended April 30,1928; 370 0. G. 757) This application is made under the act of March 3, 1883, as amended by the act of April 30, 1928, and the invention herein described and claimed, if patented, may be manufactured and used by or ,for the Government for governmental purposes without the payment to me of any royalty thereon. The manner in which my process improves the art of oxidizing phosphorus vapor is illustrated by the various objects that may be accomplished by my invention.

One of the objects of my invention is to effect the oxidationof elemental phosphorus to pentavalent phosphorus without the evolution of a large yainount of heat. The oxidation of phosphorus vapor by free oxygen to phosphorus pentoxide evolves about 183,000 calories per gram molecular weight of P205 formed. On the other hand the "heat of conversion of P4 to P205 by C02 is only about 12,500 calories per mol. of P205. Accordingly, the energy that normally is evolved in the A combination of phosphorus and oxygen is conserved by'being transformed into chemical energy through the conversion of carbon dioxide to carbon monoxide.

A second object of my invention is to conserve all of the carbon monoxide originally present with the phosphorusvapor and to form as much I as 2 19, gram molecular volumes of carbon monoxide for each gram atom of phosphorus oxidized tothe pentavalent form.

A further object of my invention is to form a product that is essentially calcium metaphosphate by a process that conserves all CO originally present in the phosphorus-CO mixture, produces as 3 much as ten additional volumes of carbon monoxide for each volume of P4 oxidized to the penta- ,valent form and conserves the heat that is normally evolved by the combustion of phosphorus in air.

I It is well known that elemental phosphorus is being obtained commercially in furnaces by the reaction of carbon with phosphate rock. The phosphorus so produced passes out of thephosphorusfurnace in a gaseous mixture, containing at least 2 and gram molecular volumes of C0 for each gram atom of phosphorus vapor. Several methods have been suggested for oxidizing the phosphorus to the pentavalent form. It is common practice to burn the phosphorus mixture in 5 0 air to form. phosphorus pentoxide and carbon di-' oxide. The pentoxide may then be dissolved in water and converted in well known ways to phosphoric acid. The phosphorus'pentoxide may also be brought in contact with phosphate rock at a suitably high temperature to form a product com- 5 posed substantially of calcium metaphosphate (see U. S. Patent No. 1,925,645 and 1,925,644; also German Patent No. 541,178; 1930). This product is non-hygroscopic, contains more than P205 and is suitable for use as a phosphate fer- 10 tilizer. The preparation of calcium metaphosphate by this method is described by Curtis, Copson and Abrams (Chem. and Met. Eng. March 1937). By either of these procedures, however, the carbon monoxide present in the original phosphorus-carbon monoxide furnace gas is lost. Furthermore the oxidation of a phosphorus-carbon monoxide mixture in an excess of air evolves large amounts of heat that at times prove very bothersome. In'an endeavor to save the carbon monoxide in such a phosphate furnace gas a second method has been devised (H. A. Curtis, Chem. and

. Met. Eng. 42; June 1935), comprising the separation of phosphorus from the carbon monoxide by condensation followed by combustion of the condensed phosphorus in air. This method still entails a large evolution of heat but does conserve the carbon monoxide. A third method that has been suggested in a number of patents (German Patents 531,498, 1931; 540,068, 1931; 528,504, 1931; French Patents 624,438, 1927; 640,287, 1928), involves the oxidation of phosphorus to oxides of phosphorus by carbon dioxide added in sufiicient quantities to the gaseous mixture of phosphorus vapor, CO, and other gases normally present in phosphate furnace gas. Experimental work that I have carried out shows, however, that any attempt to oxidize phosphorus vapor by causing it to react with only carbon dioxide cannot lead to the production of phosphorus pentoxide as a sole 40 product. An equilibrium exists in the reaction P2O4+CO2 CO+P2O5 in the range above 900 such that a mixture of P204 (phosphorus tetroxide) and P205 is obtained. This mixture of oxides cannot easily be converted into pure phosphoric 45 acid because the tetroxide reacts with water to form phosphorus acid as well as phosphoric acid. Hence, unless some additional process is resorted to for oxidizing the tetroxide or phosphorous acid,

this third process for oxidizing phosphorus is not 5 very useful in those cases in which pure phosphoric acid or phosphates (free of phosphorous acid or phosphites) are desired as products.

I have discovered a new and useful process for oxidizing phosphorus in a gas mixture such as is commonly evolved from phosphate furnaces. For example, I have found that if a suitable mixture of phosphorus vapor, C0, C02 and the usual fur-- nace gas impurities is passed into a bed of phosphate rock at some high temperature, preferably about 1200 0., all of the phosphorus of the gas mixture is oxidized to the pentavalent form and combines with the phosphate rock to form substantially calcium metaphosphate together with 2 gram molecular weights of carbon monoxide for each gram atomic weight of phosphorus in the original gas mixture. The action can be explained in connection with the equation written above. The phosphate rock combines with the phosphorus pentoxide thereby removing it from the equilibrium mixture CO2--P2O4-COP2O5 allowing in consequence additional P204 to be oxidized by carbon dioxide to phosphorus pentoxide, this latter in turn combining with phosphate rock. In such a manner phosphorus and its lower oxides are substantially eliminated, being converted into the pentavalent form in calcium metaphosphate.

A typical procedure for carrying out my process for the oxidation of phosphorus with the formation of the calcium metaphosphate is as follows: A mixture of phosphorus vapor, carbon monoxide,

and carbon dioxide either with or without additional gases is passed into some suitable solid reactant, such as phosphate rock, preferably at a temperature in excess of 980 C. If no oxygen is present, the entering gas mixture must contain at least 2 gram molecular volumes of carbon dioxide for each gram atomic weight of elemental phosphorus. To facilitate oxidation it is even better if this ratio is as high as 5:1. Such a mixture could be made by adding about 200 volumes of carbon dioxide gas to each 100 volumes of a (JO-phosphorus gas mixture used, if the latter has the usual composition of about 9% P4 and 90% GO. If the percentage P4 in the gas is smaller than 9% less CO2 will of course have to be added.

' The above representation describes a typical procedure for effecting the oxidation of phosphorus by carbon dioxide in the presence of an excess of phosphate rock to a product that is substantially calcium metaphosphate. Attention should be directed to the fact that the phosphate rock is being used as a reactant and not merely as a catalyst. Sufficient phosphate rock must be brought continuously in contact with the carbon dioxide-phosphorus mixture to react with allthe phosphorus pentoxide stoichiometrically equivalent to the original phosphorus vapor. Numerous variations of my procedure may be devised, which still incorporate the essential features of the method here proposed by having carbon dioxide as the oxidizing agent and by having a reactant present that is capable of combining preferentially with the pentoxide (rather than the tetroxide) of phosphorus thereby causing all the tetroxide to be oxidized over to the pentoxide as explained in detail above. One variation that might be incorporated would consist of adding some oxygen or air to the original phosphoruscarbon monoxide mixture. As long as the oxygen thus added is not sufiicient to oxidize the phosphorus and the CO completely to phosphorus pentoxide and CO2, respectively, the method is essentially the same as that proposed here, be-

cause in contact with the phosphate rock or other solid reactant one will have an equilibrium mixture of P204-COCO2P2O5 from which the phosphate rock or other solid reactant will remove the P205 as explained above and the carbon dioxide Will then act as the oxidizing agent in con verting the phosphorus tetroxide to phosphorus pentoxide. Of course, if some 02 is added to the gas, the percent of CO in the exit gas will be smaller than if no 02 were added. Furthermore, it does not matter if the phosphorus is partially oxidized to various of its oxides before being brought in contact with the phosphate rock in the presence of carbon dioxide sufficient in quantity to efiect complete oxidation of phosphorus and its lower oxides to pentavalent phosphorus. Similarly the presence of the various impurities that are usually present along with phosphorus vapor and carbon monoxide in. gases coming from electric or blast furnaces used for the reduction of rock phosphate to phosphorus, do not interfere with the method here proposed. Another variation in the rnethod consists in substituting another reactant for phosphate rock. Any of the high melting calcium compounds such as CaSOi or CaCOa can be substituted for phosphate rock, if desired, and still effect the complete oxidation of the phosphorus to the pentavalent form, since these materials are capable of combining preferentially with phosphorus pentoxide in the presence of phosphorus tetroxide to form calcium metaphosphate and let the carbon dioxide react with the phosphorus tetroxide to convert it completely to the pentoxide, which in turn is converted into calcium metaphosphate. Furthermore, other reactants than calcium compounds may be used to shift the equilibrium in the P204CO-CO2-P205 mixture by combining with or dissolving the P205 preferentially with respect to P204 at high temperature. Silica and alumina are two such materials. The choice of the solid reactant will be dictated by the usefulness of the solid phosphate formed and by the capability of the solid reactant combining with or dissolving the P205 preferentially with respect to P204.

Having thus described my invention, what I claim for Letters Patent is:

l. The method of oxidizing phosphorus vapor, consisting of subjecting phosphate rock at a temperature of at least 900 C. to the action of a mixture of CO2 and phosphorus vapor in which the ratio of the CO2 to phosphorus is greater than 2%; gram molecular volumes of carbon dioxide per gram atomic weight of elemental phosphorus.

2. The method of oxidizing the lower oxides of phosphorus, consisting of subjecting phosphate rock at a temperature of at least 900 C. to the action of a mixture of CO2 and the oxides of phosphorus in which the concentration of CO2 is greater than that stoichiometrically necessary for the oxidation of the lower oxides of phosphorus to pentavalent phosphorus.

3. The method of oxidizing phosphorus vapor, consisting of subjecting phosphate rock at a temperature of at least 900 C. to the action of a mixture of CO2, 02, CO, and phosphorus vapor in which at least the stoichiometric quantity of CO2 and 02 for oxidizing the phosphorus to the penta- Valent form is present, and in which the quantity of O2 is not sumcient to oxidize both the phosphorus and CO to pentavalent phosphorus and CO2, respectively.

the lower oxides of phosphorus to the pentavalent' form is present, and in which the quantity of 02 present is not sufiicient to oxidize both the phosphorus and the C0 to pentavalent phosphorus and CO2, respectively.

PAUL H. EMIWETI'.